${10}^5$ coloumb charge liberated 1 gm silver (Ag). If the charge is doubled
then the amount of liberated Ag will be:

The concentration of $ZnC{l}_2$ solution will change when it is placed in a container which is made of:

The cell reaction of an electrochemical cell is \(Cu^{2+}(C_{1}) + Zn \to Cu + Zn^{2+}(C_{2})\).

The change in free energy will be the function of:

\(1. \ ln (C_{1}+C_{2})\)
2. \(ln (\frac{C_{2}}{C_{1}})\)
\(3. \ ln C_{2}\)
\(4. \ lnC_{1}\)

The value of E⁰ cell for the following reaction is:
\(Cu^{2+}+ Sn^{2+}\to Cu +Sn^{4+ } \)

(Given, equilibrium constant is 10⁶)

For the disproportionation of copper:

2Cu⁺ → C u²⁺ + C u$,$ $E°$ is:
(Given $E°$ for Cu⁺²/Cu is 0.34 V & Eº for Cu⁺²/Cu⁺ is 0.15 V )

1. 0.49 V

2. – 0.19 V

3. 0.38 V

4. – 0.38 V

A cell reaction become spontaneous when:

1. ∆Gº is negative

2. ∆Gº is positive

3. $E_{Red}^{°}$ is positive

4. $E_{Red}^{°}$ is negative

At infinite dilution, equivalent conductances of Ba⁺² & Cl^– ions are 127 & 76 ohm^–1cm^–1 eq^–1 respectively. Equivalent conductance (ohm^–1cm^–1 eq^–1) of BaCl₂ at infinite dilution is:

1. 139.5

2. 101.5

3. 203

4. 279

In electrolysis of NaCl when Pt electrode is taken then H₂ is liberated at the cathode while with Hg cathode it forms sodium amalgam because:

In the silver plating of copper, K[Ag(CN)₂] is used instead of AgNO₃. The reason is:
 

Consider the following  reaction:

$\frac{\mathrm{}}{}$\(\frac{4}{3} \mathrm{Al}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \frac{2}{3} \mathrm{Al}_2 \mathrm{O}_3(\mathrm{~s})\), $∆\mathrm{G}=-827$ $\mathrm{KJ}$ ${\mathrm{mol}}^{-1}$

The minimum e.m.f. required to carry out the electrolysis of Al₂O₃ is:
(F = 96500 C mol^–1)

1. 2.14 V

2. 4.28 V

3. 6.42 V

4. 8.56 V